Hydrogen oxidation and generation over carbon films

ABSTRACT

An electrode comprises an acid treated, cathodically cycled carbon-comprising film or body. The carbon consists of single walled nanotubes (SWNTs), pyrolytic graphite, microcrystalline graphitic, any carbon that consists of more than 99% sp 2  hybridized carbons, or any combination thereof. The electrode can be used in an electrochemical device functioning as an electrolyser for evolution of hydrogen or as a fuel cell for oxidation of hydrogen. The electrochemical device can be coupled as a secondary energy generator into a system with a primary energy generator that naturally undergoes generation fluctuations. During periods of high energy output, the primary source can power the electrochemical device to store energy as hydrogen, which can be consumed to generate electricity as the secondary source during low energy output by the primary source. Solar cells, wind turbines and water turbines can act as the primary energy source.

CROSS-REFERENCE TO RELATED APPLICATION

The present application claims the benefit of U.S. Provisional Application Serial No. 61/424,323, filed Dec. 17, 2010, which is hereby incorporated by reference herein in its entirety, including any figures, tables, or drawings.

BACKGROUND OF INVENTION

Restraining the widespread use of solar cells and windmills for power generation is the problem that energy demand does not vary in the manner of the availability of sunlight and wind. Therefore, an efficient means of storing and releasing energy during periods of excess and insufficient generation by these sources is needed for the promotion of these natural renewable energy sources. Coupling an unreliable primary generator to a regenerative fuel cell can perform that function. The regenerative fuel cell operates by storing energy by the generation of hydrogen via the electrolysis of water and releasing energy upon demand by oxidation of the hydrogen, generally regenerating water. By using one or more fuel cells matched in capacity to the primary power generator, a reliable system can result. Fuel cells are attractive because they can be compact and can possess a low internal resistance.

Present cells, capable of performing this function, generally rely on the use of platinum as an electrocatalyst. Unfortunately, platinum is of insufficient supply to make this a viable option for large scale application of the technology. State of art electrodes use precious metal catalysts for the generation and oxidation of hydrogen since non-noble metal electrocatalysts exhibit corrosion in acidic or other environments under which these reactions are carried out. Additionally, noble metals electrodes often exhibit performance degradation with time due to the loss of electrochemical surface area because the finely divided particles agglomerate.

An article entitled: “From Hydrogenases to Noble Metal-Free catalytic nanomaterials for H₂ Production and Uptake”, Le Goff et al. Science, 326, 1384 (2009), reports that hydrogen (H₂) generation results from water electrolysis and hydrogen oxidation over a nickel complex based electrocatalyst supported on multiwall carbon nanotubes (MWNTs). Control experiments, reported therein, indicate that MWNTs do not function as an effective electrocatalyst for either hydrogen generation or oxidation, and catalytic currents observed for the subject electrocatalyst during H₂ oxidation and generation can be attributed solely to the Nickel complex supported by the MWNTs.

Other alternates to Pt have been examined as electrocatalysts for the formation of H₂. Yang et al., Synthetic Metals 154, 69 (2005) entitled: “Hydrogen Generation using PPy-FMS modified PVDF Membrane and Other Substrates,” reports the polypyrrole containing catalytic ferrocene centers can increase electrocatalyst' s conversion current compared to Pt. Unfortunately, it was concluded that a Pt supporting electrode is required for observation of long-term stability as deposition of the polypyrrole on stainless steel results in catalytic properties vanishing after just a few hours. The reverse reaction, H₂ oxidation, is not disclosed in Yang et al.

Winther-Jensen et al., Adv. Mater. 22, 1727 (2010) entitled: “Conducting Polymer Composite Materials for Hydrogen Generation,” reports hydrogen generation from aqueous acidic electrolyte solution using a conducting polymer composite, comprising poly(3,4-ethylenedioxythiophene) (PEDOT) polymerized on a polytetrafluoroethylene (PTFE) membrane in the presence of polyethylene glycol (PEG), as the electrocatalyst. Catalytic activity of the PEDOT-PEG composite improved after 24 hour immersion in 1 M sulfuric acid with the increased activity attributed to the swelling of the composite by that electrolyte solution. The overpotential observed for the composite electrode was higher than that observed with Pt. The reverse reaction, H₂ oxidation, is not reported in Winther-Jensen et al.

Carbon has been extensively studied as a catalyst support in the hydrogen evolution reaction (HER) and the hydrogen oxidation reaction (HOR). Although carbon appears to synergistically enhance the activity of the metallic catalysts for HER and HOR, carbon electrodes that are free of metallic catalysts are reported to promote HER only at a high overpotential but are not reported to promote HOR. Prosini et al., J. Power Sources 118, 265-269 (2003) disclose that carbon nanotube films produce hydrogen but required a significant overpotential for hydrogen oxidation. Misra et al., ACS Nano 3, 3903-3908 (2009) disclose that MWNTs displayed hydrogen evolution at a voltage of −10 V and is silent on HOR.

As stated in Kinoshita, K., Carbon: Electrochemical and Physicochemical Properties (Wiley, New York, 1988): “The hydrogen overpotential on most graphite and carbon surfaces is high; consequently these materials, by themselves, are not useful electrodes for hydrogen oxidation/evolution.”; and “. . . carbon does not have electrochemical activity for the electrochemical oxidation of H₂.” To this end, an electrode comprising an effective non-noble metal, stable electrocatalyst that exhibits little or no overpotential during the generation or oxidation of H₂ remains a goal.

BRIEF SUMMARY

Embodiments of the invention are directed to an electrode for an electrochemical cell that comprises a carbon-comprising film or body, for example, single walled carbon nanotube (SWNT) or graphite, where a portion of the carbon comprising film or body consists of at least 99% sp² carbons that has undergone an activation process consisting of exposure to oxidizing acids along with some cathodic electrochemical cycling. In an embodiment of the invention, a thin carbon-comprising film can be combined with a porous support, such as a porous polytetrafluoroethylene (PTFE), polyvinylidene fluoride (PVDF), polyethylene, polypropylene, polyester, polyamide, carbon paper, or other porous membranes. The carbon-comprising film can be as thin as about 20 nm up to a thickness of 100 μm.

Embodiments of the invention are directed to electrochemical devices comprising at least one electrode comprising an activated carbon-comprising film or body. The electrochemical device can perform a hydrogen evolution reaction (HER) in an electrolyzer mode and can perform a hydrogen oxidation reaction (HOR) in a fuel cell mode. In another embodiment of the invention, the electrochemical device can be a component of a sustainable electrical energy storage/generation system. The system employs a primary energy generator driven by a natural renewable energy source, which does not combust a fuel, where the primary energy source is coupled to a secondary energy generator that is the electrochemical device according to an embodiment of the invention. The secondary energy source functions as an electrolyser to store energy from this primary source as hydrogen, when the primary electrical energy generator generates energy in excess of the demand upon the system, and functions as a fuel cell to consume the hydrogen with the generation of electricity, when the conditions do not permit the primary system to generate sufficient energy for the demand upon the system. Primary energy generators can be solar cells, wind turbines, or water turbines.

BRIEF DESCRIPTION OF DRAWINGS

FIG. 1A shows a top view of an exemplary electrochemical cell, according to an embodiment of the invention, used to examine the hydrogen oxidation reaction (HOR) and hydrogen evolution reaction (HER).

FIG. 1B shows a side view of the exemplary electrochemical cell of FIG. 1A, according to an embodiment of the invention, used to examine the hydrogen oxidation reaction (HOR) and hydrogen evolution reaction (HER).

FIG. 2 is plots of current density versus potential for HER in 1M sulfuric acid for an electrode comprising a 1.5 μm thick SWNT film, according to an embodiment of the invention, scanned at 5 mV/s after 0 (top curve), 4, 48, 96, and 120 (bottom curve) hours of acid exposure and a few (<10) cathodic scan cycles from +0.2 to −0.7 V versus an NHE reference electrode, scanning at 50 mV/s between each recorded curve.

FIG. 3 displays current density versus potential plots for HER using an electrode of 0.106 mg/cm² of Pt metal sputtered onto a PTFE membrane (curve that touches the y-axis) and an electrode of 0.106 mg/cm² SWNT film on a PTFE membrane after a 120 hour treatment with 1 M sulfuric acid, according to an embodiment of the invention.

FIG. 4 is chronoamperometry plots for a three terminal measurement of a working electrode comprising a SWNT film where a high HOR activity occurs following treatment of the electrode with the 1 M sulfuric acid electrolyte for 288 hours, according to an embodiment of the invention, and for the same SWNT film prior to acid treatment where the working electrodes are exposed to alternating H₂ and Ar atmospheres, for the films with and without acid treatment.

FIG. 5 shows measurements for a rotating ring-disk electrode (RRDE), according to an embodiment of the invention, confirming that the cathodic currents are due to hydrogen evolution where the ring electrode was held at +0.6 V as the activated SWNT film on the disk electrode was swept between ±0.2 V, at 5 mV/s, where the coincidence of the ring current with the disk current indicates oxidation of the hydrogen evolved at the disk.

FIG. 6 is a plot of current density versus potential for HOR (positive potentials with respect to NHE) and for HER (negative potentials with respect to NHE) for the electrode comprising an acid treated SWNT film of FIG. 4, according to an embodiment of the invention, and for a commercially available Pt loaded gas diffusion electrode.

FIG. 7 is a plot of the HER current for the 27 μg activated SWNTs on the glassy carbon disk RRDE of FIG. 5, measured in a 1 M H₂SO₄ solution at 1400 rpm with a scan rate of 50 mV/s, which achieves a 58 mA/cm² current density at 200 mV overpotential (a specific activity of 422 A/g), according to an embodiment of the invention.

FIG. 8 is a plot of the HER and HOR currents over a 10 hour period for an activated SWNT film (54 μg) using a Teflon electrochemical cell, according to an embodiment of the invention, exposed to a 1 M H₂SO₄ solution at +300 and −300 mV, respectively.

FIG. 9 shows cyclic voltammograms (CV) measured in an electrochemical cell employing an acid activated 1.5 μm thick SWNT film, according to an embodiment of the invention, in pH 7.2 phosphate buffer (0.6 M) (left curve) and with a commercial Pt loaded GDE under the same conditions.

FIG. 10 shows a CV plot (50 mV/s scan rate) for a device with an electrode having an activated SWNT film (54 μg) in pH 6.4 buffer (3 M) using a stirred solution where the onset of HER occurs at ˜30 mV overpotential.

FIG. 11 shows the Faradaic efficiency for HER of the acid activated SWNTs comprising an electrode using a stirred unbuffered KCl solution at −1.4 V, where the measured pH values (squares) are contrasted with calculated pH values (triangles) for the solution based on the measured charge (inset).

FIG. 12 shows a CV plot for an activated SWNT film (27 μg on a 5 mm diameter glassy carbon disk electrode, static measurement) for HER in filtered, additive free, Atlantic seawater (St. Augustine Beach, Fla.), according to an embodiment of the invention, where the inset shows the forward sweep of the current on a log scale to facilitate identification of the onset potential, −570 mV, indicating an overpotential of ˜68 mV, as evaluated using the solution pH measured at the end of the CV measurement.

FIG. 13 shows the effect of CO exposure on the HOR for a Pt loaded GDE and an electrode comprising an acid activated SWNT film at 50 mV overpotential in 1 M H₂SO₄ where the rapid recovery of the SWNT HOR activity demonstrates that conventional metals are not responsible for catalytic activity, in accordance with the embodiment of the invention.

FIG. 14A shows CV plots for HER using films comprising SWNTs activated in 1 M nitric acid, according to an embodiment of the invention, with the HER currents measured at the indicated times.

FIG. 14B shows CV plots for HER using films comprising SWNTs activated in 1 M hydrochloric acid, according to an embodiment of the invention, with the HER currents measured at the indicated times.

FIG. 15 shows overlapping Raman spectra of the D and G band regions for a nanotube film before and after acid activation, where spectra are normalized to the same G-band peak intensity.

FIG. 16 is a polarization curve for an electrode comprising an acid treated SWNT film, according to an embodiment of the invention, used as an HOR anode in a hydrogen-air fuel cell, according to an embodiment of the invention.

FIG. 17 shows CV plots for HER currents versus potential, as a function of time in 1 M nitric acid, for a piece of highly ordered pyrolytic graphite (HOPG) possessing a basal plane face area of 5.8 cm² and thickness of 0.23 mm, according to an embodiment of the invention.

FIG. 18 shows CV plots for HER evolution current of an electrode comprising the activated piece of HOPG of FIG. 17, in pH 6.3 phosphate buffer (3 M) displaying a near zero onset overpotential)(E° for the reaction.

FIG. 19 shows CV plots for HER as a function of exposure time to 1 M nitric acid for a 3.18 mm diameter graphite electrode rod after exposure for 0, 2, 4, 24 and 48 hours.

DETAILED DISCLOSURE

It has been discovered that by exposing carbon materials, where at least portions thereof consists of more than 99% sp² hybridized carbons, to acids that are intercalants of graphite while undergoing low voltage cathodic cycling, form carbon materials that are highly active as HER and HOR electrodes that initiate at near zero overpotentials. These electrodes comprising acid treated carbon materials display activities that can exceed the activity of the best known non-precious metal catalysts for HER and HOR. The high activity for HER persists in pH neutral water and in sea water. Although most of the disclosure herein is directed to exemplary embodiments employing single wall carbon nanotubes (SWNTs), in embodiments of the invention, other carbon materials consisting of more than 99% sp² bonded carbons, such as highly ordered pyrolytic graphite and sintered microcrystalline graphite can be included in the effective catalysts towards HER and HOR, which display high activity and nearly zero overpotential. Although exemplary embodiments are directed toward films, the electrodes need not be a film, but can be a body of any shape which may be configured to possess a high degree of open porosity making a large surface area accessible by electrolytes. A nearly zero overpotential is one where the onset overpotential is less than about 10 mV in a strong acid (pH 1 or less) and about 70 mV in a pH neutral (pH 7) electrolyte. In contrast, catalytic activity has not been observed for acid treated glassy carbons, where the overpotential for observation of HER remains over 500 mV in strong aqueous acids.

Embodiments of the invention are directed to electrodes having an electrocatalyst for hydrogen (H₂) generation and oxidation that comprises a carbon-comprising film, for example, a single walled carbon nanotube (SWNT) film, where the overpotential for generation of H₂ is nearly zero. During studies on uses of SWNTs, it was discovered that SWNT film electrodes can have a high oxygen reduction activity; similar to platinum (Pt), but no catalytic activity was observed for SWNT films toward HOR. However, studies of oxygen reduction in sulfuric acid using SWNTs indicated that proton reduction currents accompanying hydrogen evolution increased over time. Further study revealed that after exposure of SWNT films to an acid electrolyte with a few low voltage cathodic cycles, the H₂ evolution reaction (HER) initiates at zero overpotential. The overpotential is the difference between the observed applied potential required for a reaction to occur and the thermodynamic potential for the reaction. Exposure of H₂ to the electrode comprising acid treated SWNT films, according to an embodiment of the invention, results in a facile hydrogen oxidation reaction (HOR) that exceeds the efficiency disclosed for the Ni complex supported on MWNT, which is disclosed in Le Goff et al. The HER activity of electrodes comprising acid exposed SWNT films also exceeds that of commercially available Pt-loaded electrodes on a mass basis.

An electrode, according to an embodiment of the invention, is fabricated employing the deposition of a SWNT thin film in the manner disclosed in U.S. Pat. No. 7,261,852, which is incorporated in its entirety herein. By this method, a suspension of SWNTs in water using a surfactant is vacuum filtered onto the surface of a filtration membrane having pores that are too small for penetration of the SWNTs into the pores. After removal of the aqueous portion of the suspension, SWNT bound surfactant is washed from the film and the film is dried. The film can vary, as required, in surface area and thickness. The film porosity can be increased by a number of means, including those disclosed in U.S. Pat. No. 7,704,479, incorporated in its entirety herein. The geometric surface area is determined by the size of the surface of the filtration membrane to which the suspension is provided and through which the aqueous solution is passed. Any portion of a filtration membrane can be use, and, in some embodiments of the invention, less than 100 percent of the membrane surface is used. In an embodiment of the invention, a HOR electrode is formed such that hydrogen accesses the acid treated SWNT film through the pores of the filtration membrane, which is tolerant of an acidic electrolyte. The membrane can be hydrophobic. The film comprises a plurality of SWNTs that are oriented with their long axis approximately parallel to the adjacent surface of the membrane, with the nanotubes randomly oriented within the local plane of the film, such that there is intimate electrical contact, generally with intimate physical contact, between nanotubes over the entire surface of the film. In this manner, the electrical conductivity over the entire film can be high for a very thin film, for example having a thickness of about 20 nm to about 200 nm in thickness. Thick SWNT films, for example, up to 1 to 100 μm or more, can be used, and bodies having dimensions in excess of 100 μm can be used.

In embodiments of the invention, acid treatment for activation of the SWNT comprises contacting the SWNT film with an acid solution for a sufficient period of time with a number of cathodic cycles induced over the course of the exposure . The number of cycles necessary to induce the activity being less than 100. The solution can be an aqueous solution or a non-aqueous solution. The time required for activation depends on the concentration and strength of the acid. An exemplary activated film has been treated with an aqueous 1 M sulfuric acid solution for 120 hours. Other strong acids can be used at higher and lower concentrations, as can be appreciated by one skilled in the art. Other Brønsted acids can be used, for example, nitric acid, perchloric acid, trifluoroacetic acid, trifluoromethanesulfonic acid, perfluorobutanesulfonic acid, boric acid, iodic acid, and periodic acid. In other embodiments of the invention, the acid can be a Lewis acid, for example, metal chlorides, bromides, fluorides and oxyhalides such as AlCl₃, AlBr₃, FeCl₃, AsF₅, and SbCl₅.

When employed as a HER electrode, a porous membrane can allow egress of the H₂ produced. The electrode includes an electrical contact to the carbon-comprising film. For example, a SWNT film can be deposited on a portion of a porous disk and an electrical conductor, for example, a metal, can be formed on another portion of the filtration membrane that overlaps onto the portion having the carbon-comprising film. For example, a metal can be deposited by any of various techniques, such as sputtering, evaporation or electrolytic deposition, on a specific portion of the carbon-comprising film. The hydrophobic filtration membrane can be polytetrafluoroethylene (PTFE), polyvinylidene fluoride (PVDF), polyethylene, polypropylene, polyester, polyamide, porous carbon paper, or any other membrane. In other embodiments of the invention, the porous membrane can be a polymer generally considered hydrophilic where the surface has been treated to achieve a hydrophobic surface. In other embodiments of the invention, the membrane can be a porous glass or ceramic that can be inherently resistant to wetting or can be treated to generate a hydrophobic surface. For example a sintered glass membrane can be surface treated with a silane coupling agent to render the surface hydrophobic and poorly wettable by an aqueous solution.

The HOR rate observed for an electrocatalytic acid treated SWNT film, according to an embodiment of the invention, can be optimized by maximizing the three phase interface between H₂, the SWNT film electrode, and the electrolyte solution. Optimization can be carried out as disclosed in International Publication No WO 2010/126767, Nov. 4, 2010, and incorporated herein by reference, for the use of pure SWNT films for oxygen reduction. According to embodiments of the invention, hydrogen diffuses through the pores of the membrane to a three phase interface, where the hydrogen gas, the solid SWNT film and the liquid electrolyte are present. At this three phase interface, hydrogen dissolves into the surface layer of electrolyte solution and is oxidized upon contact with the SWNT film electrode, providing electrons to the external circuit through the SWNT film. When the acid contacted SWNT film is used as an anode for hydrogen oxidation in combination with a SWNT oxygen reducing cathode, as disclosed in WO 2010/126767, a completely metal catalyst free hydrogen-oxygen fuel cell is constructed according to an embodiment of the invention.

According to an embodiment of the invention, an electrochemical device comprising the electrode comprising an acid treated carbon-comprising film is included to form a sustainable energy storage/generation system in conjunction with a primary renewable energy generator. Because natural renewable energy conversion by primary sources, such as solar and wind sources by a solar cell or wind turbine, are, by their nature, irregular and unpredictable, the energy from this primary source in excess of that immediately consumed, when conditions are favorable for generation, is stored as hydrogen that is produced via electrolysis of water in an electrolyser coupled to a gas storage device. Subsequently, when the primary energy source is insufficient for achievement of the energy demand, the electrolyser runs in reverse as a fuel cell to supply needed energy. In an embodiment of the invention, the primary natural energy source can be reliable, such as a hydroelectric source using a water turbine, but has extended periods where the energy generated or consumed are excessive or insufficient, respectively, for example, during the day and night in a residence. By coupling of the primary source to the electrochemical device comprising the electrode comprising an acid treated carbon-comprising film or body, hydrogen can be generated at low energy demand, such as during the night, and stored for supplementation of the primary energy source during peak demand, for example, at peak activity times during the day.

Methods And Materials

To examine the acid treated SWNT film electrodes for HER and HOR, SWNT films were deposited on oversized 47 mm diameter PTFE filtration membranes as 15 mm diameter disks off-set to one side of the supporting membrane. Electrical contact to the SWNT film was made by sputtering a 200 nm thick layer of Pd through a rectangular shadow mask to cover from the edge of the bare membrane to the nanotube film, overlapping about ˜2 mm of the 15 mm diameter SWNT film.

FIGS. 1A and 1B illustrate a cross section of a metal contacted carbon-comprising film, for example, a SWNT film, on a porous membrane 102/101/103 situated in a cell used to test the electrochemical performance of the electrocatalyst in a cell for H₂ formation and/or oxidation, according to an embodiment of the invention. The electrode has a SWNT film 101, a contact electrode 102 and an underlying porous hydrophobic membrane 103. The cell body 104 was fabricated from a solid rectangular PTFE block (3.6 cm×3.6 cm×5.6 cm), with a 2.54 cm diameter hole bored from the top (along the long axis) to create a 4.6 cm deep electrolyte reservoir 105. A 0.76 cm diameter opening 106 through the cell sidewall accesses the reservoir 105 for electrolyte within the cell. An O-ring 107 surrounds the sidewall opening 106 in the cell and forms a leak free seal against the SWNT film 101 of the SWNT film/electrode/membrane assembly 102/101/103 when the PTFE membrane 103 supporting the SWNT film 101 and electrode 102 are pressed against the O-ring 107 by a gas flow cover 108, which is fabricated from a material such as, in this example, Plexiglass. The metallic electrode 102 is located outside the electrolyte wetted region defined by the opening 106. The SWNT film/electrode/membrane assembly 102/101/103 held by the Plexiglass gas flow cover 108 is secured to the cell body 104 by screws (not shown) through holes 109 at its 4 corners. In a working cell, the O-ring 107 can be replaced with a crimp seal, epoxy cement, adhesive or curing sealant. The gas flow cover 108 incorporates a gas plenum 112 that when secured to the cell body 104 positions the plenum in line with opening 106.

H₂ gas is fed to and from the plenum 112 by ports 110 and 114, respectively, which are situated on either side of the plenum 112 to which they are connected through holes 111 and 113, respectively. For experimental purposes, outlet 113 allows gas to exit into a water bubbler to prevent ambient atmosphere from entering the system. The hydrophobic PTFE membrane 103 prevents the electrolyte from flowing out of the cell, while allowing diffusion of H₂ to the electrolyte wetted SWNT film 101 in the HOR mode. In the HOR mode, the hydrogen is adsorbed, dissociated and oxidized to protons (H⁺) with the transport of the electrons formed to the SWNT film 101 and to the external circuit through the metal electrode 102. In the HER mode, power is supplied to the SWNT cathode 101/102/103 by a voltage against a Pt counter electrode 121 (the anode) controlled with respect to a reference electrode 122, which are situated in a tight fitting cover 123 for three terminal measurements. At the anode 121, water is oxidized to liberate oxygen and protons that diffuse through the electrolyte. Protons are reduced to hydrogen at the SWNT cathode leading to H₂ gas evolution.

For three terminal measurements, a blank glass slide 117 is placed across the second sidewall hole in the cell sealing against the O-ring 116 by pressure from the blank cover 118. The blank cover 118 is secured against the cell body by 4 screws (not shown) that go through 4 holes in the blank cover (two indicated). The cell has a tight fitting cover 123 that has feed through holes for the counter and reference electrodes 121 and 122, respectively, and also a feed through hole for a purge tube 120 to bubble inert gas into the electrolyte and an outlet hole for the purge gas (not shown). In a two terminal measurement mode, a second gas flow cover identical to 108 is used over the second sidewall opening 115.

Rotating ring-disk electrode (RRDE) measurements were performed using a Pine Instruments AFCBP1 Bipotentiostat, AFMSRCE Rotator with an E6 series RRDE with a Pt ring and glassy carbon disk. Linear sweep and cyclic voltammograms, measured in the specially constructed electrochemical cell, were recorded using a Gamry Reference 600 Potentiostat. Faradaic Efficiency measurements were performed in the RRDE set-up, keeping the solution well stirred by rotating at 1600 rpm. A Denver Instrument model 220 meter was used for pH measurements.

HER activity of the acid treated SWNT films was studied in 1 M sulfuric acid for successively increased exposure times of the SWNTs to the acid electrolyte. FIG. 2 shows plots of HER current density versus potential determined using three terminals measurements with a 1.5 μm thick SWNT film, 54 μg of SWNTs, on 0.22 μm pore Teflon membrane, scanned at 5 mV/s following 0, 4, 48, 96 and 120 hours of acid exposure using a Ag/AgC1 (3 M KCl) reference electrode. FIG. 2 shows potentials plotted relative to the normal hydrogen electrode (NHE) by addition of 210 mV to the Ag/AgCl (3 M KCl) reference electrode value. As clearly shown in FIG. 2, the HER activity of the SWNT film increased dramatically with the acid exposure time over more than 48 hours, while the overpotential for HER gradually decreased to zero (relative to a normal hydrogen electrode (NHE)) with increasing acid exposure time. As a reference for the low onset potential of the HER, FIG. 2 plots the HER current for the cell using a 50 nm thick Pt film sputtered onto the PTFE membrane as a replacement for the SWNTs electrode. FIG. 3 shows the HER activity relative to the Ag/AgCl (3 M KCl) reference electrode in 1 M sulfuric acid for the 1.5 μm thick SWNT film after 120 hours of exposure to 1 M sulfuric acid and for the HER activity of the 50 nm thick pure platinum film in contact with 1M sulfuric acid for 120 hours. The Pt film activity did not vary with acid exposure time. Both measurements were conducted with scanning at 5 mV/s.

The necessity for acid treatment of SWNTs films for HOR electrocatalysts is shown in FIG. 4, where the SWNT film was activated by H₂SO₄ exposure and used in three terminal Chronoamperomtry measurements employing a 1.5 μm thick SWNT film on a PTFE membrane as the working electrode. The 1 M sulfuric acid electrolyte solution was held at +0.3 V versus NHE. The gas being fed through the gas plenum 112 to the SWNT film 101 through the PTFE membrane 103, as shown in FIGS. 1A and 1B, was varied between H₂ and argon, as indicated in FIG. 4. Prior to activation of the SWNT film by contacting with acid, no current was observed, regardless of the gas fed to the electrode. In contrast, after the SWNT film had been exposed to the 1 M sulfuric acid, in this example for 288 hours, a rapid response with a substantial current density in the presence of H₂ is observed.

FIG. 5 shows rotating ring-disk electrode (RRDE) data where SWNTs (27 μg) were drop cast from ethanol onto a 5 mm diameter glassy carbon disk electrode followed by activation in 1 M H₂SO₄ for 144 hr prior to recording the data shown. Control experiments on the glassy carbon disk electrode without nanotubes confirmed an overpotential for HER that remains high, about −500 mV vs. NHE, under similar conditioning. The measurements confirm that cathodic currents are due to proton reduction (with H₂ evolution). Measurements were recorded in 1 M H₂SO₄ with the ring rotating at 1200 rpm. The disk potential was linearly swept at 5 mV/s between ±0.2 V, as shown in the bottom plot. The center plot shows the disk reduction current, while the top curve shows the oxidation current from the Pt ring held at +0.6 V, detecting the hydrogen. With the disk held stationary, H₂ bubbles evolve from the nanotube layer at −60 mV, becoming increasingly vigorous with increasing overpotential. The saturation seen in the hydrogen oxidation ring current is due to the increasing number of H₂ bubbles that physically separate the electrolyte from the ring on their excursion outwards. The larger current dips correspond to the separation of particularly large bubbles.

Electrocatalytic activity towards HOR and HER of a SWNT film (1.5 microns thick, 0.106 mg/cm²) after 12 days exposure to 1 M H₂SO₄ was measured as a function of applied potential against a Pt counter electrode and referenced to a NHE electrode. In like manner, the same measurements were made using a commercially available, optimized, Pt loaded carbon electrode (BSAF ELAT GDE, 0.5 mg/cm²) that, for the purpose of wetting to maximize its performance, had the potential cycled between +0.2 to −0.5 V for ˜10 cycles over the course of a few minutes. The potential cycling increased the HOR and HER currents for the Pt comprising electrode by a factor of about two, which did not further increase with additional cycling or after additional time in the 1 M sulfuric acid. FIG. 6 shows the logarithmic current density as a function of overpotential in the electrochemical cell for an activated SWNT film (54 μg) measured in 1 M H₂SO₄ (5 mV/s scan rate) with H₂ flowing through the gas plenum (bottom curve). For comparison, the SWNT film was replaced with a Pt loaded (0.5 mg/cm², 250 μg Pt exposed to the electrolyte) commercial gas diffusion electrode (ELAT HT140EW, The Fuel Cell Store) and measurements were recorded under the same conditions with the platinized microporous layer facing the electrolyte (top curve). The activated SWNT electrode exhibits the transition from HER to HOR at zero overpotential, as does the Pt loaded GDE, corroborating the low overpotential for initiating the reactions on the activated SWNTs. At −200 mV overpotential, the HER current for the SWNTs is a remarkable 30 mA/cm², versus 86 mA/cm² for the Pt loaded GDE. At this overpotential the specific (mass basis) activity of the SWNTs is 278 A/g, which exceeds that 172 A/g determined for the Pt loaded electrode under these conditions. The hydrogen oxidation current at +200 mV is only slightly less remarkable for the SWNT film at 7 mA/cm², having a specific activity of 65 A/g compared to the Pt electrode's specific activity of 168 A/g under the same conditions.

The commercial Pt electrode is highly engineered to maximize its three phase interface (catalyst-electrolyte-gas). In contrast, the acid activated SWNT film was not modified to enhance its activities. SWNTs under these conditions tend to be hydrophilic compact films that possess small-channel tortuous-path porosity. For the HOR reaction, the compactness and hydrophobicity makes relatively little of the SWNT film's thickness accessible, which, when combined with the relatively low solubility of hydrogen in acid, makes these results very impressive. Therefore, a more engineered film or support with improved porosity and hydrophobicity should produce even more impressive activities. Similarly, H₂ bubbles trapped on and within the film pores tend to block regions of the SWNTs film, which can be engineered for greater activity. This is consistent with the data shown in FIG. 7, using the RRDE, where the 27 μg, acid activated SWNT layer rotating at 1400 rpm attains 58 mA/cm² of HER current at −200 mV (vs. NHE), which corresponds to 422 A/g. The improvement, over the specific activity of 278 A/g for the measurement performed using the stationary electrode used in FIG. 2, results from the facile removal of the hydrogen bubbles by rotation to avoid hydrogen occluded electrode area.

For comparison, at −200 mV (+200 mV), a nickel bisdiphosphine catalyst (Le Goff et al., Science, 2009, 326, 1384-1387) exhibits a hydrogen evolution (oxidation) current of ˜1.3 mA/cm² (0.9 mA/cm²) for 60 μg/cm² of the catalyst, yielding a specific activity of 22 A/g (15 A/g). Amorphous molybdenum sulfide films (Merki et al., Chem. Sci., 2011, 2, 1262-1267) exhibit HER current densities disclosed be “among the highest reported for non-noble catalysts” display 14 mA/cm² at −200 mV, which is about a factor of two lower than the

SWNT HER activity for the SWNT films according to an embodiment of the invention. Measurements carried over a 10 hour period, as shown in FIG. 8, demonstrate that the high activity is retained over the duration of the measurement for the SWNT HOR and HER at +300 and −300 mV, respectively. The apparent slow decay observed in FIG. 8 for the HOR activity is consistent with a confinement effect of the protons generated within the SWNT films, as indicated by interruption of the current, after which, HOR activity returns to its original value.

The films are useful for hydrogen production from pH 7 water. FIG. 9 shows HER curves for the CVs of an acid activated SWNT film (top) and the Pt loaded GDE (bottom) using a pH 7.2 phosphate buffer (0.6 M). In FIG. 9, solid tangent lines were drawn to aid in estimation of the points where HER initiates for the electrodes, which are indicated by dashed vertical lines, which occur at ˜420 mV for the Pt loaded electrode and at ˜490 mV for the activated SWNT film with a remarkably low overpotential for the onset of only ˜70 mV. The SWNT film displays a HER current of 22 mA/cm² at an overpotential of 1 V. The larger separation of the forward and reverse parts of the scan for the commercial Pt electrode reflects the larger non-Faradaic capacitive charging due to the greater surface area of the commercial electrode compared to the relatively compact SWNT film. As shown in FIG. 10, HER for the SWNTs in a 3 M pH 6.4 buffer displays an onset at an overpotential of only 30 mV and yields 38 mA/cm² of HER current at 1 V overpotential. The lower onset potential, relative to that for the 0.6 M pH 7.2 buffer, occurs because the higher salt concentration reduces the cell's IR drop, while stirring reduces effects due to concentration polarization. Increasing noise, at higher currents, is consistent with periodic disturbance of the bubbles that form at the film surface, as the “noise” stopped when the stirring was turned off. The switch to the higher current path corresponds to a large bubble being detached from the film surface.

Table 1, below, compares the overpotential for reaction onset and the current density at the given overpotential at near neutral pH for the SWNT catalyst, according to an embodiment of the invention, with reported values for the best non-precious metal catalysts. A separate measurement of the pH change, in initially near neutral, non-buffered, 1 M KCl solution, confirms hydrogen evolution with 100% Faradaic efficiency. FIG. 11 shows the measured changes in pH with time (squares) and the calculated pH (triangles) based on the corresponding measured charge (inset), assuming that each pair of electrons corresponds to the evolution of one hydrogen molecule and a hydroxyl ion that raises the pH. Hydrogen evolution from filtered Atlantic seawater (without additives) is plotted in FIG. 12, demonstrating that the activated SWNT electrodes are tolerance to impurities and are robust.

TABLE 1 Non-precious-metal HER overpotential for the onsets and activities near pH 7: Reaction Current Catalyst onset OP^(a) density @ OP^(a) Reference Nickel^(II)- cyclam ~0.90 V   ~10 μm/cm² @ 1 V b, c Cobalt pentapyridine 0.66 V 2.4 mA/cm² @ 0.9 V d Molybdenum-oxo 0.52 V 9.1 mA/cm² @ 1 V e complex Activated SWNT 0.03 V 38 mA/cm² @ 1 V ^(a)overpotential; b Collin et al., Inorg. Chem., 1988, 27, 1986; c Cook, et al., Chem. Rev., 2010, 110, 6474; d Sun, et al., J. Am. Chem. Soc. 2011, 133, 9212; d Karunadasa et al. Nature, 2010, 464, 1329.

Transmission electron microscopy (TEM) images of purified SWNT material show an occasional opaque particle characteristic of nickel and cobalt metals, which are used as growth catalysts for SWNT synthesis. The quantity of the metals is below the detection limits (0.1 At. %) of an XPS measurement that was performed. Moreover, Pourbaix diagrams (Beverskog et al., Corros. Sci, 1997, 39, 969-980 and Powell et al., J. Chem. Educ., 1987, 64, 165-167), suggest these metals can only survive the SWNT purification (HNO₃ reflux), H₂SO₄ acid exposure, and the test conditions if encased in bucky-onions, that would render the metal surfaces inaccessible as the catalytic sites. Conclusive demonstration that conventional metals are responsible for the observed activity is shown in FIG. 13, where the carbon monoxide sensitivity of the HOR activity for the activated SWNTs is indicated. The HOR current normalized to the initial current, at 50 mV overpotential for the Pt loaded commercial GDE in 1 M H₂SO₄, displays poisoning upon the addition of 500 ppm CO to the hydrogen flowing through the gas plenum, where the electrode remains inactive after the CO flow is terminated and 100% H₂ feed is restored. The acid activated SWNT film shows deactivation with the very high CO concentration; however, after the CO flow is terminated and the 100% H₂ feed is restored, HOR activity immediately begins to recover. All conventional metal catalysts would have been rendered inactive by the CO exposure.

Sulfuric acid is a known spontaneous “intercalant” in SWNTs bundles. To test whether intercalation is relevant to the activity enhancement, activation of samples was attempted in 1 M HNO₃ and 1 M HCl, the former, a known charge transfer intercalant of sp² bonded carbons while the latter is not. Acid exposure and low voltage cycling gave only a small increase of the HER currents in HCl while activation in the HNO₃ was comparable to that in the H₂SO₄, as shown in FIGS. 14A and 14B. Exposure to higher concentrations of HNO₃ (6 M and 16 M) greatly accelerated the rate of the activation. SWNTs exposed to 16 M HNO₃ for 8 hrs and transferred to 1 M HNO₃ for cycling and measurements attained saturation HER currents (for any given voltage) within 8 hrs in the 1 M acid. Raman spectra of acid activated and non-activated SWNT samples are shown in FIG. 15. Spectra were recorded in a Renishaw Ramascope 1000, using 532 nm excitation and 1 mW power. Four spectra were recorded at distinct positions of the film within the region that had been exposed to the acid during cycling, the region bounded by the o-ring (activated region), and four spectra were recorded at distinct positions well outside the region defined by the o-ring (non-activated region). Besides a consistent peak upshift and a reduced D/G band ratio in the spectra from the activated region, the activated region spectra are consistently lower in intensity by a factor of ˜1.6, providing further evidence for the intercalation, as the resonant Raman intensity depends on the real electronic transition rate, which is reduced by a partial ground state depletion upon charge transfer intercalation. Given the consistent differences between the spectra in the two regions, the four spectra common to each region were summed and normalized to the same g-band peak intensity giving the results shown in FIG. 15. The Raman spectra display an upshift in the G band of 2.6 cm⁻¹, consistent with a moderate degree of intercalation upon activation. The D/G band ratio in these samples shows a small decrease of the ratio in the activated sample, as is evident from the relative intensities of the D bands in FIG. 15 where the spectra were normalized to the same G band peak intensities. This Raman spectral evidence strongly indicates that the activation does not induce defects or effect chemical functionalization of the nanotube sidewalls. Although acid treatment might effect chemistry at the pre-existing nanotube ends and defects, the activity does not appear to require defects, as the activity observed for microcrystalline graphitic carbon films, which contain far more edge sites per volume than there are nanotube ends in the SWNT films, is not in excess of that observed for SWNT films.

The SWNT film was tested as a hydrogen oxidizing anode in a hydrogen-air fuel cell configuration in a two terminal mode employing an electrochemical cell using both sidewall openings and a second gas plenum cover. The 1.5 μm thick SWNT film on a PTFE membrane, disclosed above, was situated over one sidewall opening, and an air cathode was situated over the second sidewall opening. The air cathode consisted of a half membrane electrode assembly (MEA) with a Pt (1.0 mg/cm²) loaded gas diffusion electrode painted with a Nafion solution subsequently bonded to one side of a Nafion 212 membrane. The Nafion membrane contacted the 1 M sulfuric acid electrolyte in the cell to serve as a barrier to cross-over of any unreacted gasses that made it through the two electrodes, which is a probable situation during testing under high impedance loading of the cell when low currents are drawn from the fuel cell. The SWNT film anode was fed H₂ gas flowing through its associated plenum at a low flow rate, while the MEA was simply exposed to air by leaving the fittings to its plenum open to the ambient environment. The anode was connected to the cathode through a variable resistor. Voltage across the resistor and current through the circuit was monitored as the resistance was decreased. FIG. 16 shows the resulting polarization curve constructed from the monitored voltage and resistance.

Highly ordered pyrolytic graphite (HOPG) was examined to test the activity of other sp² carbon-comprising bodies, using random cuttings of high quality (low mosaic spread) HOPG, from the fabrication of X-ray monochromator crystals (Union Carbide, Ohio). Additionally, a microcrystalline graphitic rod was examined with a sample from Bay Carbon (grade ST-21), having impurities reported to be 1 ppm Si, and <1 ppm of Al, Ca, B, Fe and Mg. Evolution of the HER currents versus potential as a function of time in 1 M nitric acid for a piece of highly ordered pyrolytic graphite possessing a basal plane face area of 5.8 cm² and thickness of 0.23 mm is shown in FIG. 17. HER evolution current of the activated HOPG sample in pH 6.3 phosphate buffer (3 M) is shown in FIG. 18. Remarkably, the onset overpotential (E°) is nearly zero for the reaction at this pH. FIG. 19 shows the evolution of the HER currents versus potential as a function of time in 1 M nitric acid for a 3.18 mm diameter graphite electrode rod.

All patents, patent applications, provisional applications, and publications referred to or cited herein are incorporated by reference in their entirety, including all figures and tables, to the extent they are not inconsistent with the explicit teachings of this specification.

It should be understood that the examples and embodiments described herein are for illustrative purposes only and that various modifications or changes in light thereof will be suggested to persons skilled in the art and are to be included within the spirit and purview of this application. 

We claim:
 1. An electrochemical cell, comprising: an anode comprising a carbon-comprising body, wherein at least a portion of the carbon material of the carbon-comprising body consists of more than 99% sp² hybridized carbons and wherein the carbon material has undergone a plurality of low voltage cathodic cycles in the presence of an acid to form an electrode configured to perform a hydrogen evolution reaction (HER) and a hydrogen oxidation reaction (HOR); and a cathode comprising a carbon-containing electrocatalyst configured to perform oxygen reduction.
 2. A method of forming an electrode, comprising: exposing a carbon material of a carbon-comprising body to an acid, wherein the carbon material comprises single-walled carbon nanotubes (SWNTs), double-walled carbon nanotubes (DWNTs), multiwalled carbon nanotubes (MWNTs), graphene, pyrolytic graphite, and/or microcrystalline graphite; and subjecting the carbon material to a plurality of low voltage cathodic cycles in the presence of the acid to form an electrode configured to perform a hydrogen evolution reaction (HER) and a hydrogen oxidation reaction (HOR).
 3. The method of claim 2, wherein the carbon material comprises single-walled carbon nanotubes (SWNTs).
 4. The method of claim 2, wherein subjecting the carbon material to the plurality of low voltage cathodic cycles in the presence of the acid comprises exposing the carbon material to acid for at least 48 hours.
 5. The method of claim 2, wherein subjecting the carbon material to the plurality of low voltage cathodic cycles in the presence of the acid comprises subjecting the carbon material to voltage cycling within a range between voltage values that are a fraction of a volt (V).
 6. The method of claim 2, wherein the onset overpotential is less than 10 mV where an electrolyte solution has a pH equal to or less than 1 and less than 70 mV where an electrolyte solution has a pH equal to
 7. 7. The method of claim 2, wherein the carbon-comprising body is a carbon-comprising film having a thickness of 20 nm to 100 μm.
 8. The method of claim 2, wherein the method further comprises depositing the carbon-comprising body as a carbon-comprising film on a porous membrane.
 9. The method of claim 8, wherein the porous membrane is configured to support the carbon-comprising body and the carbon-comprising body comprises single walled carbon nanotubes (SWNTs).
 10. The method of claim 8, wherein the porous membrane comprises polytetrafluoroethylene (PTFE), polyvinylidene fluoride (PVDF), polyethylene, polypropylene, polyester, polyamide, or porous carbon paper.
 11. The electrochemical cell of claim 1, wherein the anode comprises single walled carbon nanotubes (SWNTs).
 12. The electrochemical cell of claim 1, wherein the anode further comprises a porous membrane configured to support the carbon-comprising body, and wherein the carbon-comprising body is a carbon-comprising film.
 13. The electrochemical cell of claim 12, wherein the porous membrane comprises polytetrafluoroethylene (PTFE), polyvinylidene fluoride (PVDF), polyethylene, polypropylene, polyester, polyamide, or porous carbon paper.
 14. The electrochemical cell of claim 1, wherein the carbon-comprising body is a carbon-comprising film having a thickness of 20 nm to 100 μm.
 15. The electrochemical cell of claim 1, wherein the carbon material has been exposed to the acid for at least 48 hours.
 16. The electrochemical cell of claim 1, wherein the plurality of low voltage cathodic cycles includes voltage cycling within a range between voltage values that are a fraction of a volt (V).
 17. The electrochemical cell of claim 1, wherein the onset overpotential is less than 10 mV where an electrolyte solution has a pH equal to or less than 1 and less than 70 mV where an electrolyte solution has a pH equal to
 7. 